D and F block elements
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3d series is from
SC to zn
4 d series is from
Y to Cd
5 d series is from
La and Hf to Hg
6 d series is from
Ac and elements from Rf to Cn
The element which does not have electrons in s orbital during ground state
Pd
Which orbital protrude to the periphery very much and hence are more influenced by surroundings
D orbital
Ions of d^ n configuration show similarity in
Magnetic and electronic properties
In any row of d block elements the melting points of these metals rise to a maximum at d^5 but the exceptions are
Mn and Tc
A very important factor that determines the standard electrode potential is
Enthalpy of atomization
High enthalpy of atomization means
High boiling point
Metals with high enthalpy of atomization tends to be
Noble in their reaction
Which series of d block have more enthalpy of atomization
2d and 3d ( graph in ncert)
The factors affecting ionization enthalpy is
Attraction btw nucleus and electron Repulsion btw Electrons Exchange energy
In p block which oxidation state is favoured by heavier members
Lower oxidation state ( inert pair effect)
In d blocks which oxidation state is found to be stable for heavier members
High oxidation state
Copper is inable to liberate H2 from acids because of
Positive electrode potential
Which acids react with Cu
Nitric acid and hot concentrated sulphuric acid
For which all elements electrode potential is more negative than expected
Mn, Ni and Zn
Beyond Mn which all have trihalides
Fe and Co
Why is Cu(2+) more stable than Cu(1+) in aqueous solution ?
Because of more negative hydration enthalpy
The metals of first series are reactive the exception to this is
Cu
Ti(2+) , V(2+) and Cr(2+) are
Strong reducing agents
Mn(3+) , Co(3+) are
Strong oxidizing agents
The catalyst btw iodine and persulphate ions
Fe (3+)